**Equilibrium Constant and Concentrations in a Chemical Reaction**The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-2} \) at 698K:\[ 2 \text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g) \]If an equilibrium mixture of the three gases in a 10.8 L container at 698K contains 0.413 mol of HI(g) and 0.348 mol of H₂, the equilibrium concentration of I₂ is \(\_\_\_\_\_\_\_\) M.**Note:**- \( \_\_\_\_\_\_\_\) represents a blank space to be filled with the concentration value.- Use the following steps to calculate the equilibrium concentration: 1. Convert the moles of gases to molarity by dividing by the volume of the container (10.8 L). 2. Apply the equilibrium constant expression: \[ K_c = \frac{[\text{H}_2][\text{I}_2]}{[\text{HI}]^2} \] 3. Solve for the unknown concentration.

Answered: Image /qna-images/answer/103ee424-510b-4356-8cbc-4cb3fa65b527.jpg

The equilibrium constant, K., for the following reaction is 1.80×102 at 698K. 2HI(g)H2(g) + I2(g) If an equilibrium mixture of the three gases in a 10.8 L container at 698K contains 0.413 mol of HI(g) and 0.348 mol of H2. M. the equilibrium concentration of I, is

The equilibrium constant, K., for the following reaction is 1.80×102 at 698K. 2HI(g)H2(g) + I2(g) If an equilibrium mixture of the three gases in a 10.8 L container at 698K contains 0.413 mol of HI(g) and 0.348 mol of H2. M. the equilibrium concentration of I, is

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The reaction is investigated (assume an ideal gas mixture): 3N2(g) + 2H2O(g) – 2N¿0(g) + N½H«(g) Initially there are 4.0 moles of H2O and 2.0 moles of N2, in a 2.0 L container. If the concentration of N2O at equilibrium is 0.30 M, what is the molar concentration of H2O at equilibrium? (A) 0.15 M (B) 0.30 M (C) 1.7 M (D) 1.9 M
The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH3(g) + H₂S(g) NH4HS(s) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.366 mol NH4HS, 1.34×10- M NH3 and 1.34×10-² M H₂S. If the concentration of NH3(g) is suddenly increased to 2.41x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] = ΣΣ M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCI3(g) + Cl₂(g) PCI5(g) Calculate the equilibrium concentrations of reactant and products when 0.587 moles of PCI3 and 0.587 moles of Cl₂ are introduced into a 1.00 L vessel at 500 K. [PCI3] = [Cl₂] [PCI 5] = = M M M
The equilibrium constant, K. , for the following reaction is 1.80x10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) If an equilibrium mixture of the three compounds in a 6.85 L container at 298 K contains 1.56 mol of NH HS(s) and 0.468 mol of NH3, the number of moles of H,S present is moles.
The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl(g) COCI,(g) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of CO and 0.451 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] [Cl] [COCL,] = MMM
q The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. [Review Topics] [References] Use the References to access important values if needed for NH4HS(9) NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.322 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M Submit Answer Show Hint NOV 30 Le... The equilib tv Retry Entire Group 9 more group attempts remaining Email In M
A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…
Please dont provide handwrittin solution....
The equilibrium constant, K. , for the following reaction is 7.00x105 at 673 K. NH,I(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 6.89 L container at 673 K contains 2.67 mol of NH,I(s) and 0.210 mol of NH3, the number of moles of HI present is moles.